In the equilibrium N_2 + 3H_2 rightleftharpoo | vedclass

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(A) The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 22 \ kcal$.
This is an exothermic reaction $(\Delta H < 0)$ where

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Increasing the pressure

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(A) The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 22 \ kcal$.
This is an exothermic reaction $(\Delta H < 0)$ where the number of moles of gaseous products $(2)$ is less than the number of moles of gaseous reactants $(1 + 3 = 4)$.
According to Le Chatelier's principle,for a reaction with a decrease in the number of moles,increasing the pressure will shift the equilibrium in the forward direction to reduce the pressure.
Therefore,the formation of ammonia is favoured by increasing the pressure.

In the equilibrium $N_2 + 3H_2 \rightleftharpoons 2NH_3 + 22 \ kcal$,the formation of ammonia is favoured by

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